Acetylene gas, c2h2, can be produced by the reaction of calcium carbide and water. cac2(s) + 2h2o(l) --> c2h2(g) + ca(oh)2(aq) how many liters of acetylene at 742 mm hg and 26c can be produced from 2.54 g cac2(s)?

1.0 L

Explanation:

Given that:-

Mass of =

Molar mass of = 64.099 g/mol

The formula for the calculation of moles is shown below:

Thus,

According to the given reaction:-

1 mole of on reaction forms 1 mole of

0.0396 mole of on reaction forms 0.0396 mole of

Moles of = 0.0396 moles

Considering ideal gas equation as:-

where,

P = pressure of the gas = 742 mmHg  

V = Volume of the gas = ?

T = Temperature of the gas =

R = Gas constant =

n = number of moles = 0.0396 moles

Putting values in above equation, we get:

1.0 L of acetylene  can be produced from 2.54 g .

"hydrogen bonding is the attraction of h atoms in the water molecule (slight + charge) to o atoms in a neighboring water molecule (slight - charge); it is a weak interatomic force. but it is still strong enough to the water molecules "stick" together."

every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. therefore, there must be the same number of atoms of each element on each side of a chemical equation.